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Chapter 8: Q9 E (page 446)

Why is the concept of hybridization required in valence bond theory?

Short Answer

Expert verified

Hybridization is necessary to determine the molecular geometry of complex.

Step by step solution

01

Definition of Concept

Hybridization occurs when two or more different pure orbitals with comparable energy are mixed together to produce an equivalent amount of impure orbitals with equal energy and definite geometry, which are referred to as hybrid orbitals.

02

Explain why is the concept of hybridization required in valence bond theory

Hybridization: Hybrid orbitals are created when two or more different pure orbitals with comparable energy are mixed together to produce an equivalent amount of impure orbitals with equal energy and definite geometry. This phenomenon is known as hybridization. It uses the valence bond theory of orbitals to help determine molecular geometry.

Therefore, the molecular geometry of complexes must be determined through hybridization..

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Most popular questions from this chapter

Explain why bonds occur at specific average bond distances instead of the atoms approaching each other infinitely close.

Label the molecular orbital shown as σ or Π, bonding or antibonding, and indicate where the node occurs.

Write Lewis structures for \({\rm{N}}{{\rm{F}}_{\rm{3}}}\) and \({\rm{P}}{{\rm{F}}_{\rm{5}}}\). On the basis of hybrid orbitals, explain the fact that \({\rm{N}}{{\rm{F}}_{\rm{3}}}\), \({\rm{P}}{{\rm{F}}_{\rm{3}}}\), and \({\rm{P}}{{\rm{F}}_{\rm{5}}}\) are stable molecules, but \({\rm{N}}{{\rm{F}}_{\rm{5}}}\) does not exist.

For each of the following molecules, indicate the hybridization requested and whether or not the electrons will be delocalized: (a) ozone (\({{\rm{O}}_{\rm{3}}}\)) central \({\rm{O}}\) hybridization (b) carbon dioxide (\({\rm{C}}{{\rm{O}}_{\rm{2}}}\)) central \({\rm{C}}\) hybridization (c) nitrogen dioxide (\({\rm{N}}{{\rm{O}}_{\rm{2}}}\)) central \({\rm{N}}\) hybridization (d) phosphate ion (\({\rm{P}}{{\rm{O}}_{\rm{4}}}^{{\rm{3 - }}}\)) central \({\rm{P}}\) hybridization.

A useful solvent that will dissolve salts as well as organic compounds is the compound acetonitrile, \({{\rm{H}}_{\rm{3}}}{\rm{CCN}}\). It is present in paint strippers. (a) Write the Lewis structure for acetonitrile, and indicate the direction of the dipole moment in the molecule. (b) Identify the hybrid orbitals used by the carbon atoms in the molecule to form \({\rm{\sigma }}\) bonds. (c) Describe the atomic orbitals that form the \({\rm{\pi }}\) bonds in the molecule. Note that it is not necessary to hybridize the nitrogen atom.
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